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Joe Meza
Hope Smith

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When you chemically combine these two atoms, the Sodium atom is giving an electron to the chlorine atom. The Sodium atom losses an electron and fills its outer most level, then chloride receives an electron which also fills the electron outermost level. Sodium becomes a cation and chloride becomes an anion.

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Fluorine atom received an electron from another atom and became a Fluorine ion.

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1. Metals - lose electrons to form positive ions (cations)
2. Nonmetals - gain electrons to form negative ion (anions)
3. The difference between an ion and an atom is the number of ELECTRONS
4. The more electrons the atom has the more spaced out it will become
5. The charge of electrons will be found in the upper right hand corner (superscript)
6. If you put a (-) in the charge you are gaining electrons
7. Ions can be negative or positive
8. The difference between protons and electrons is the protons will never change
9. First group = +1
Second group = +2
Aluminum = +3
10. Ionic compounds are made up from metals and nonmetals
- metals are always listed 1st nonmetals 2nd
- all metals are (+), nonmetals (-)
11. Ratio is subscript
__# of metals__ (charge) + __# of nonmetals__ (charge) = 0
ex.  S & Al
Sulfide Aluminum      __3__ (-2) + __2__ (+3) = 0
-6         +        6      = 0
S(3)Al(2)

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Red, Orange, Yellow Green - Metals
Blue- Metalloids
Dark Blue, Purple - Non metals

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The difference between these Hydrogen Atoms is the atomic mass. They are all the same element because the protons stay the same, the only thing that changes in the number on neutrons. The first Hydrogen atom (Protium) has 1 proton and 0 neutrons. The second Hydrogen atom (Deuterium) has 1 proton and 1 neutron, showing that it is still a hydrogen atom. The third Hydrogen atom (Tritium) has 1 proton and 2 neutrons, the element is still Hydrogen just with a different number of neutrons.

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This is a chemical reaction between 2 atoms of Hydrogen and one atom of Oxygen . These two atoms are chemically combined, they make a new substance but  the same molecules are still present. The mass of both the reactant and the product are the same.

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1. The table lists all known elements in order of atomic number, in columns depending on similarities in the chemical and physical properties
2. It is used to identify  properties of elements, understand properties of molecules
3. Elements with similar properties are called groups (families)
4. Two numbering conventions are used to label the groups
5. Older convention - uses Roman Numerals I through VIII followed by A or B
6. Other convention - numbered groups 1 - 18
7. The "A" groups are known as "Main Group Elements"
- The "B" groups also known as "transition Elements"
8. The horizontal rows, called periods are numbered 1 - 7
- Periods all have the same energy level
9. The periodic Table is divided into 3 categories
- Metals, located in the left and center of the table. They are good conductors of heat  and electricity, malleable, ductile, lustrous, and mostly solid at room temperature (except Hg, Mercury)
- Nonmetals, located in the upper right hand corner. They are poor conductors of heat and electricity, lacking most of the properties that metals have
- Metalloids, they are 6 elements on a diagonal line, called semimetals or    semiconductors because there conductivity is between metals and nonmetals
10. Most elements are very reactive, generally combined
11. Noble gasses and gases are found uncombined (gold,, platinum, silver)
12. Diatomic molecules are two of the same atoms bonded together

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1. Atoms make up everything around us

2. The relative mass of proton and neutron = 1

3. The relative mass of an electron is 0

4. The majority of mass in an atom is in the nucleus

5. The atomic mass unit (amu) = the subatomic particles

6. 1amu = the mass of the proton + neutron (relative)

7. The mass of atom = mass of protons and neutrons

8. Atomic mass, average of all the different isotopes not including electrons

9. Mass number, protons + neutrons

10. Atomic # = 3 of protons

11. Mass number is not on the periodic table, protons = the neutrons

12. Isotopes = the same # of protons, different number of neutrons

13. Subscript - small # below or to the right of an atom, many of the atom are connected in a molecule

14. Coefficient - large # in front of an atom or molecule (# of copies)

15. Letters - each atom alone or combined, 1 capital letter, tells you the name of the atom

16. The arrangement of the atoms is determined by the physical and chemical properties

17. If they have subscripts they are also bonded

18. ex. Each molecule of a compound that has been implicated in the formation of acid rain contains one atom of sulfur and three atoms of oxygen                   SO(3)

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1. The diameter of an atom is 10,000x larger than the diameter of the atomic nucleus
2. The subscript tells you the atomic number, the number of protons and electrons if the atom is neutral
3. The superscript tells the mass number and the number of protons and neutrons
4. The electrical charge is "0" if the atom is neutral
5. You can identify an isotope by the element name - mass #
ex. Sodium - 24
6. All isotopes have the same atomic number because they all have the same # of protons
7. All isotopes don't have the same mass # because the neutrons differ
8. Isotope - an atom of an element with the same # of protons and different mass # and neutrons

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August 30, 1871, Brightwater, New Zealand

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December 18, 1856, Cheetham Hill, Manchester, United Kingdom

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John Dalton was born September 6, 1766, in Eaglesfield, England

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1. Used the gold foil experiment to discover positively charged particles

2. He shot alpha particles (+) at a piece of gold foil

3. The results were that most of the alpha particles went through the foil without being deflected, others were scattered, and few were shot straight back

4. He discovered positive particles in the atom, also known as the nucleus

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1. Used a cathode ray tube and a magnet to discover a negative charge in atoms

2. The tube is a closed, gas, vacuumed tube

3. He discovered smaller particles in an atom that are negatively charged

4. They are called electrons, a subatomic particle

5. He was the first scientist to make a model of the atom, called the “Plum Pudding model”

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1. First scientist to use “data”

2. If you start with the same substance you can end with something different

3. All elements are composed of atoms

4. Law Of Conservation Of Mass - mass of the product = the mass of the reactants

5. Law Of Multiple Proportions - same substance stays the same as what they are divisible by, same ratio

6. *Atom = indivisible, can’t be divided, can’t be created or destroyed in chemical reactions*

7. Compounds are composed of different elements

8. *Atoms of the same element are identical*